1. Using one set of data from Table 1 above, calculate the molar absorptivity of the Cr3+ solution using equation 1. Hint: rearrange the Beer-Lambert Law to solve for a. The pathlength is 1.0 cm and the units of molar absorptivity will be cm'M1. 2. Using the molar absorptivity value calculated in question 1 above, determine the absorption of a solution with a concentration of Cr* of 0.0325 M.
1. Using one set of data from Table 1 above, calculate the molar absorptivity of the Cr3+ solution using equation 1. Hint: rearrange the Beer-Lambert Law to solve for a. The pathlength is 1.0 cm and the units of molar absorptivity will be cm'M1. 2. Using the molar absorptivity value calculated in question 1 above, determine the absorption of a solution with a concentration of Cr* of 0.0325 M.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Could you help me with the questions needed to start these two questions. I’m a little confused on where to begin.
Transcribed Image Text:1. Using one set of data from Table 1 above, calculate the molar absorptivity of the Cr3+ solution
using equation 1. Hint: rearrange the Beer-Lambert Law to solve for a. The pathlength is 1.0
cm and the units of molar absorptivity will be cm 'M1.
2. Using the molar absorptivity value calculated in question 1 above, determine the absorption of a
solution with a concentration of Cr3* of 0.0325 M.
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Concentration of CR3+ in solution (m)
Absorbance (A)
0.01
0.162
0.02
0.326
0.03
0.509
0.04
0.678
0.05
0.83
Calculating Molar Absorptivity
0.9
0.8
y= 16.88x -0.0054
0.7
0.6
0.5
0.4
0.3
0.2
*******-
0.1
0.01
0.02
0.03
0.04
0.05
0.06
Concentration of Cr 3+ in solution (m)
Series1
. Linear (Series1)
8
Sheet1 +
Calculation Mode: Automatic
Workbook Statistics
Absorbance (A)
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